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Periodic Table (Trends (Electronegativity (Electronegativity is the…
Periodic Table
Trends
Electronegativity
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Electronegativity increases from left to right on the periodic table because the number of protons increases, causing there to be a stronger pull on the electrons
First Ionization Energy
First ionization energy is the energy required to move the most loosely bound electron (highest energy electron) from a neutral atom to form a cation
First ionization energy increases from left to right on the periodic table because electronegativity increases and more energy is required to remove an electron.
First ionization energy increases from down to up on the periodic table because there is less shielding, which makes the pull on electrons stronger and causes the need for more energy to remove an electron.
Atomic Radius
Atomic radius increases going down any group in the periodic table because an atom gets bigger as more electron shells are added.
Atomic radius decreases going from left to right on any period on the periodic table because there are more protons being added while electrons are being added to the same energy level. The greater nuclear charge causes a stronger attraction of electrons, pulling them closer to the nucleus and decreasing the atom in size.
Atomic radius is the distance between the center of the nucleus of an atom to the boundary of the electron cloud of an atom.
Electron Affinity
Electron Affinity increases from left to right across periods because electronegativity increases and there is a stronger pull on electrons
Electron Affinity increases from down to up in groups on the periodic table because because the pull of electrons toward the nucleus gets stronger
Electron affinity is the energy change caused by an electron being added to a neutral atom to form an anion
Ions
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Nonmetals on the periodic table tend to form cations, while metals tend to form anions
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